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Can a change in a gaseous system be isobaric, isochoric, and
isothermal at the same time? Why or why not?

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(1) A given mass of gas is enclosed in a suitable container so that it can be maintained at constant volume. Under these conditions, there can be no change in what property of the gas? (a) Pressure. (b) Density. (c) Internal energy. (d) Temperature. (e) None of the above.
How would the temperature of a REAL gas (not perfect) in a reversible adiabatic expansion be affected?
(i) the temperature of T1 and T2. (ii)the work done by the gas along the path QM.
The change in the internal energy with entropy at constant volume is the inverse of temperatureTrue or False? Why?
Suppose a gas absorbs 498 J of energy while doing 147 J of work on its environment. Calculate the change in the internal energy of the gas.
Each line of the following table gives data, in Btu, for a process of a closed system. Determine the missing table entries, in Btu. Process Q a b с d e i 40 -4 -10 3 W i i 5 0 10 E₁ IN 15 7 -10 8 E₂ H Mi 14 -8 ΔΕ i 30 10
(a) An ideal gas is taken through a quasi-static process described by P = av, with a = 5.50 atm/m, as shown in the figure. The gas is expanded to twice its original volume of 1.00 m3. How much work (in MJ) is done on the expanding gas in this process? P P= aV? 1.00 m3 2.00 m3 MJ (b) What If? How does the work done in part (a) compare to the lowest and highest possible amounts of work that can be done on this gas between the initial and final states if the pressure always remains between P, and P and the volume always remains between V, and V2 (Enter your answers as percentages of the work done in part (a).) WIowest x 100% = W. part (a) W highest x 100% = W. part (a)